A 200 g block of an unknown metal at 150 $^\circ$C is placed into 500 g of water at 25 $^\circ$C in an insulated container. The specific heat capacity of water is $4.18$ J g$^{-1}$ $^\circ$C$^{-1}$.

(i) Assuming no heat loss to the surroundings, determine the specific heat capacity of the metal (in J g$^{-1}$ $^\circ$C$^{-1}$).

(ii) The same experiment is repeated, but the container now loses heat to the surroundings at a constant rate of 10 J s$^{-1}$ for 5 minutes. Using the specific heat capacity found in part (i), calculate the final equilibrium temperature of the system (in $^\circ$C).

Question

A 200 g block of an unknown metal at 150 $^\circ$C is placed into 500 g of water at 25 $^\circ$C in an insulated container. The specific heat capacity of water is $4.18$ J g$^{-1}$ $^\circ$C$^{-1}$.

(i) Assuming no heat loss to the surroundings, determine the specific heat capacity of the metal (in J g$^{-1}$ $^\circ$C$^{-1}$).

(ii) The same experiment is repeated, but the container now loses heat to the surroundings at a constant rate of 10 J s$^{-1}$ for 5 minutes. Using the specific heat capacity found in part (i), calculate the final equilibrium temperature of the system (in $^\circ$C).

Accepted Answer

c_metal ≈ 0.44 J g⁻¹ °C⁻¹; final temperature ≈ 28.6 °C

Neco Model Questions Vol1 2019 Physics Question 30

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